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The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom, etc. Ionization energy generally increases for every electron that is removed, and increases from left to right in the Periodic Table or if moving up the periods.
In this case, from the periodic table (or according to Mastering Chemistry) Bromine (Br) has a larger sixth ionization energy than Selenium (Se).
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What should have the larger ionization energy Se or Br?
Br has the largest I.E.
Higher ionization energy Br or Bi?
Br
What is the ionization reaction for hydrobromic acid?
HCl (aq) + H2O (L) ---------> H3O+ (aq) + Cl- (aq)
Ionization of HBr?
Dispersion forces and Dipole-Dipole Source: Mastering Chemistry
Which group of elements has very high ionization energies and very low electron affinities?
Group 8 (noble gases) have the highest first ionization energy because they are already stable and don't want to lose any electrons. Ignoring the noble gases, however, group 7 halogens (F, Cl, Br, I, etc.) have the highest first ionization energy. That's because these elements have seven valence electrons, and they don't want to give up any electrons - they want another one!
What should have the larger ionization energy Se or Br?
Br has the largest I.E.
Higher ionization energy Br or Bi?
Br
Does the element Br have the highest ionization energy?
Krypton has a higher value.
What is the ionization reaction for hydrobromic acid?
HCl (aq) + H2O (L) ---------> H3O+ (aq) + Cl- (aq)
Ionization of HBr?
Dispersion forces and Dipole-Dipole Source: Mastering Chemistry
Which group of elements has very high ionization energies and very low electron affinities?
Group 8 (noble gases) have the highest first ionization energy because they are already stable and don't want to lose any electrons. Ignoring the noble gases, however, group 7 halogens (F, Cl, Br, I, etc.) have the highest first ionization energy. That's because these elements have seven valence electrons, and they don't want to give up any electrons - they want another one!
What is the process of electron gain called?
The process of electron gain is called reduction. For example, if Br gains an electron, its oxidation number is reduced from 0 to -1, and will be written as Br-. The opposite of this (electron loss) would be called oxidation, or ionization.
Why bond energy of H-F is greater than H-Br?
pata nai
Would the Br ion be bigger than the Se ion?
No. The Se ion will be larger than the Br ion. The more negative the anion's charge, the larger the radius (more electrons = stronger repulsion between the electrons; so, more distance between them). Se would become "Se2-" as an anion, and Br would become "Br1-". Because Se's "2-" anion charge is more negative than Br's "1-" anion charge, and because Se would have more relative electrons to protons than Br, there is more repulsion between electrons, and distance, within the Se ion. So, the Se ion has a larger radius. Hope it helps.
Why do metals and non-metals usually form ionic compounds whereas two bonded non-metals are never ionic?
First an explanation in terms of ionization energy and electron affinity: Metals have low ionization energies and readily form ions. Non-metals have high electron affinities- so put them together and electron transfer is favourable. Two bonded non metals are generally covalent- their ionization energies are high. Now an explanation in terms of electronegativity (electronegativity is related to ionization energy and elctron affinity) metals have low electronegativity- non metals are comparativelly high. So electron transfer is likely. Just a cautionary word about compounds of non metals never being ionic-- what about PBr5- a binary compound of two non metals- in the solid state this has the structure PBr4+ Br-...bit of a cheat really as there is a polyatomic ion in there but it is ionic!
What has the smallest radius from I Br Br I?
Br, not Br-
Which family needs a electron to complete there outer energy level?
The Halogens F, Cl, Br, I, At
